Production of predominantly crystalline sols

ABSTRACT

The present invention relates to a method for forming a stable, predominantly crystalline sol from an acid-deficient solution of a hydrous metal oxide in which the metal is in the +4 oxidation state which comprises heating said solution to a crystallizing temperature to cause an increase in conductivity of said solution, removing anion at the crystallizing temperature to a condition of further acid deficiency at a rate which approximates the rate of release of free acid to the aqueous phase of the resultant sol, and then adjusting the anion-to-metal ratio of the sol to a desired anion-to-metal ratio.

llnite States Patent McBride et al.

PRODUCTION OF PREDOMINANTLY CRYSTALLINE SOLS Inventors: John P. McBride, Oak Ridge;

Kenneth H. McCorkle, Powell; William L. Pattison, Knoxville, all of Tenn The United States of America as represented by the United States Atomic Energy Commission, Washington, DC

Assignee:

Appl. No.: 846,835

Related U.S. Application Data Continuation-impart of Ser. No. 814,311, April 8, 1969, Pat. No. 3,629,133.

U.S. Cl. 423/261, 252/301.15 Int. Cl C0lg 43/02 Field of Search 23/354, 355;

[56] References Cited UNITED STATES PATENTS 3,375,203 3/1968 Hurley 252/301.1 3,288,717 11/1966 Morse 252/30l.l 3,367,881 2/1968 Morse 252/301.l 3,461,076 8/1969 Lloyd et al 2S2/301.1 3,361,676 1/1968 McBride et al..... 252/30l.1 S 3,629,133 12/1971 McBride et al 252/30l.1 S

Primary Examiner-Carl D. Quarforth Assistant Examiner-R. L. Tate Attorney-Roland A. Anderson [57 ABSTRACT The present invention relates to a method for forming a stable, predominantly crystalline sol from an aciddeficient solution of a hydrous metal oxide in which the metal is in the +4 oxidation state which comprises heating said solution to a crystallizing temperature to cause an increase in conductivity :of said solution, removing anion at the crystallizing temperature to a condition of further acid deficiency at a rate which approximates the rate of release of free acid to the aqueous phase of the resultant sol, and then adjusting the anion-to-metal ratio of the sol to a desired anion-to-metal ratio.

2 Claims, 2 Drawing Figures Patented Sept. 11 1973 2 Sheets-Sheet 1 523: 22255 N 6 m w INVENTORS. John P. MQBride Kenneth H. MECork/e William L. Partisan ATTORNEY.

Patented Sept. 11, 1973 2 Sheets-Sheet 2 LINE 84/ l D f 20 3O 4O 5O 60 7O TEMPERATURE, C

2 IN VENTORS.

John I? MEBride Kenn efh H. ME Cork/e BY William L. Partisan PRODUCTION OF PREDOMINANTLY CRYSTALLINE SOLS CROSS-REFERENCE TO RELATED APPLICATION This application is a continuation-in-part of our copending application Ser. No. 814,311, filed Apr. 8, 1969 now U.S. Pat. No. 3,629,133.

BACKGROUND OF THE INVENTION The invention described herein was made in the course of, or under, a contract with the United States Atomic Energy Commission. It relates to a method for forming crystalline sols from hydrous oxides and to the resulting crystalline sols produced therefrom. More particularly, the present invention is concerned with a method for preparing a predominantly crystalline sol from hydrolyzable salts of a metal which forms hydrous oxides and to the resultant predominantly crystalline sols. By a predominantly crystalline sol is meant a sol with a crystalline solid fraction consisting of from 80 to 100 percent of the total solid phase. The method of this invention is of particular utility in forming concentrated predominantly crystalline sols from a hydrolyzable salt of a tetravalent metal selected from the group consisting of zirconium, hafnium, cerium, 5f rare earth metals such as thorium, uranium, and plutonium, and mixtures thereof.

As used in this specification, true conductivity" is the specific electrical conductivity of the sol or solution in units of millimhos/cm. The term is used to emphasize that the specifications on conductivity are in absolute physical units and are not merely relative readings on an arbitrary scale. In the sol the conductivity is that of the free electrolyte and not the total electrolyte in the system.

Average crystallite size ofa sol means the apparent crystallite size of calculated from X-ray diffractometer line-broadening data using the Jones B instrument correction method. Copper Ka radiation is used and the broadening ofthe (111), (220), and (311) lines is used. When the three lines do not give the same apparent size, the sizes are averaged (but differences were seldom outside experimental error). The method of calculation is a well standardized part of routine X-ray analysis and is described in X-ray Diffraction Procedures, H. P. Klug and L. E. Alexander, John Wiley and Sons, New York (1954), and in X-ray Diffraction of Polycrystalline Materials, 11. S. Peiser, H.P. Rookby, and A..I.C. Wilson, Reinhold Publishing Corporation, New York (1960).

Degree of crystallinity ofa sol is the fraction of the solid material in the sol which is crystalline. It is deter-' mined empirically by comparison of the X-ray diffractometer curve of the sol sample with the curve obtained with a set of standards of known and constant concentration and crystallinity. Calibration curves relating net diffraction peak height over background to the concentration of crystalline oxide were obtained using fully crystalline thoria and urania sols. Comparison of the diffraction peak height over background obtained with a given sol sample with these calibration curves gives by direct interpolation the concentration of crystalline material in the sol sample. The fraction of crystalline material in the sample is then calculated by dividing the concentration of crystalline material by the total concentration ofthe same material in all forms in the sampie. The total concentration (crystalline and amorphous solids) is determined by chemical analysis.

Percent of urania in crystalline form, rather than anorphous or in solution, is determined by either of two methods: 1. Comparison of the X-ray diffractometer trace for the (111) line of the sample with the diffractometer trace for the (111) line of a urania sol which can be shown to be crystalline by agreement between the X-ray diffraction line-broadening particle size and the BrunauerEmmett-Teller (BET) gas adsorption area of gel prepared from the sol through the equation:

where: p is the density of the particle,

D is the average particle diameter, and

A is the specific surface area of gel dried from the sol. The contribution of amorphous or soluble metal species to the (111) line pattern is negligible in the concentration ranges studied.

2. Comparison of the X-ray diffractometer trace for the (111) line of the sample with the diffractometer trace for the (111) line ofa thoria sol shown to be fully crystalline by BET measurements.

The particular comparison parameter chosen was the net peak height of the diffraction line divided by the background level at lower angles than the line, designated P/B. The X-ray scan is usually run from lower to higher angles of diffraction. By standardizing sample handling and diffractometer operating procedures, a monotonic calibration function of this parameter, P/B, versus U(lV) or Th(IV) molarity of the fully crystalline standard to about fi percent level of reproducibility is obtained. The same parameter, P/B, is determined on the sample, and molarity of crystalline metal oxide in the sample is interpolated in the above function.

The calibration curves are empirical and are related to the equipment and sample preparation method used. Therefore, in all determinations a standard is submitted with the sol whose crystallinity is to be determined in order that slight variations from the calibration curves resulting from sample handling, equipment parameters, etc., may be detected and proper corrections made.

Urania standards by method 1 can be used directly when the crystallite size is the same as the sample. Thoria standards by method 2 have the advantage of air insensitivity, however, and therefore are more convenient to handle despite the correction factor required in the calibration function, as described below.

A standardized crystallinity calibration curve as shown in FIG. 1 is obtained with a urania sol which applies when a 1.85 M ThO- standard sol gives a P/B 2.9. if P/B for the thoria standard is different from 2.9, then the correct P/B for the sample is calculated from the equation: P/B m (corrected) P/B (uncorrected) (P/B- ,,,,-2.9). With the corrected value of P/B thus obtained, the value of gram moles of crystalline U0 per liter is determined from the calibration curve. Knowing (from chemical analysis) the gram moles of total U0 per liter, the percent of crystalline UO is simply obtained from the equation:

% crystallinity crystalline UO ltotal UO X I00.

The application of a similar method to a quantitative determination of uncombined MgO in Portland Cement appears in a recent publication: J. Appl. Chem., S. S. Rehsi and A. J. Majeindar, Vol. 18, p. 297, October I968.

Acid-deficient nitrate solution is used as a synonym for anion-deficient salt solution in which the principal salt is a metal nitrate. This deficiency is taken with respect to the nominal, integral valency of the metal ion; e.g., a solution having a l-molar concentration of a 4-valent metal ion and having a I-ICOO content of 0.5 M and N content of 2.0 M is acid deficient to the extent of 1.5 moles anion/mole of metal is called an acid-deficient nitrate solution because the principal anion is nitrate. Thus, in any acidor aniondeficient solution, the total anion concentration is less than is stoichiometrically required for the neutral salt.

In its process aspect, the present invention is concerned with an improved method for making metal oxide sols by a liquid-liquid extraction technique to produce sols with a high fraction of crystallinity from an aqueous solution of hydrolyzable metal salts of a metal known to form a hydrous oxide.

The production of aquasols from metal nitrate solutions by liquid-liquid extraction techniques is known and exemplified by the method disclosed in U. S. Pat. application Ser. No. 643,239, now U.S. Pat. No. 3,367,881. According to that method, a hydrous oxide, typified by uranous oxide, is converted from an aqueous nitrate solution containing tetravalent uranium to a sol by contacting said aqueous solution with an aqueous immiscible organic extractant capable of selectively removing nitrate ion from the aqueous phase to produce a nitrate-deficient solution, separating the resulting aqueous and organic phases, followed by digesting the separated aqueous phase. The resultant aged or digested solution is then treated with a second volume of the organic extractant to remove additional nitrate to a nitrate-to-uranium mole ratio of 0.15 i 0.07. The resultant aqueous sol, or aquasol, is then disengaged from the organic phase and is capable of evaporation to a uranium concentration of no more than about 1.5 molar. Product sols prepared by a sol-forming method of this type were not reproducible in their properties and exhibited widely varying degrees of stability (i.e., uncertain shelf lives).

BRIEF DESCRIPTION OF THE DRAWINGS FIG. 1 is an empirically determined calibration curve from which the percent crystallinity of a given urania sol can be determined.

FIG. 2 is a typical conductivity-temperature profile developed for a uranous nitrate solution as it is procussed to a crystalline sol.

SUMMARY OF THE INVENTION The underlying inventive concept of the product and process aspects of our invention is based on the discovcry of the causes of the variation in sol stability and on process means for insuring the formation ofa stable sol reproducibly.

We have found that the stability of a sol is related to the fraction of the dispersed oxide which is crystalline. Our findings have shown that that sol which has the highest degree of crystallinity is the most stable sol.

Acting from this discovery, we have been able to define conditions which will form highly crystalline sols in a reproducible manner.

The method by which we form highly crystalline sols in a reproducible manner is based on the discovery that nitrate-deficient solutions of metals which form insoluble hydrous oxides will rapidly form a predominantly crystalline sol over a narrow and critical range of crystallizing temperature if sufficient nitrate is extracted from the aqueous phase at a crystallizing temperature to allow the crystallization process to proceed. If the hydrolyzable ion is readily oxidized (e.g., U(IV)) nitrate removal prevents undue oxidation which, if allowed to proceed, would inhibit crystallization.

In attempting to define the mechanism of sol formation we visualize that, when a sol is formed from a metal nitrate solution of the character described, the acid-deficient aqueous phase contains an aqueous water-soluble inorganic polymer of the hydrous oxide containing nitrate and other anions (e.g., formate) and which will, in the course of time, be converted into a sol. The solid or dispersed phase of the sol which forms initially on nitrate extraction will be found to be predominantly, if not essentially all, amorphous in character and, as time passes, particularly if the aqueous phase containing the dissolved inorganic polymer is aged or digested at an elevated temperature, a small fraction of the polymer is converted to a partially crystalline but still predominantly amorphous sol with an accompanying increase in release of nitric acid to the system. The nitrate still present in the system inhibits further crystallization of the amorphous fraction and, in accordance with this invention, must be removed at the crystallization temperature in order to allow further crystallization to occur. Such a mechanism could explain why sols of varying stability are produced in a process which involves a distinct digestion or aging step. On the other hand, the method of the present invention contemplates the conversion of an aciddeficient nitrate solution directly and rapidly to a predominantly crystalline sol by removing sufficient nitrate at the crystallization temperature, to allow the amorphous polymer to convert to the crystalline state.

The onset of crystallization of the acid-deficient solution is signified by a number of distinctly identifiable signs depending on the system. In the U(IV)-nitrateformate system, crystallite formation is accompanied by a pronounced gassing, by a sudden rise in the conductivity of the solution, and, generally, by a change in color with development of the dispersed phase. Inthe uranous nitrate solution or sol, for example, the deep green color of the uranous nitrate solution changes to a black shade, evidencing formation of the uranous oxide crystalline sol. In the thorium(IV) nitrate system, gassing and color changes are not seen, but a marked change in opacity signals the onset of crystallization. In some thorium systems, opacity and color changes are seen, but not gassing. A property change common to all systems at the onset of crystallization is a release of free acid from an inorganic polymer. Hence the onset and cause of crystallization can be charted by monitoring the conductivity of the sol. As soon as a rise in conductivity is noted, the process of this invention calls for rapid nitrate removal, preferably by solvent extraction with an aqueous immiscible organic extractant capable of selectively extracting nitrate ion. The rate of free acid removal should, in the ideal case, be equal to the rate at which free acid is being released. In addition, where U(lV) is the hydrolyzable ion, the rate and amount of nitrate removal should be such as to avoid reaching a free acid level which will cause excessive conversion of uranous species to uranyl species. In general terms, the amount of uranyl formation should never be allowed to exceed more than about 15 percent of the total uranium content and preferably no more than percent. The end of the crystallization process in the case of uranium will be signified by a subsidence or termination of gassing or bubble formation, whereupon further nitrate removal is continued to a conductivity level or free acid content sufficient to stabilize the sol. In the case of uranium, the conductivity should be such as would be measured in a fully crystalline urania sol containing a nitrate-to-uranium mole ratio of 0.1 i 0.02.

Each acid nitrate-deficient metal nitrate solution will have its characteristic crystallizing temperature range. In the case of uranous nitrate solutions, a crystallizing temperature in the range of 58 to 65C. is operable, with a preferred narrower range of from 61 to 63C. The characteristic crystallizing temperature or range of temperature of any hydrolyzable metal salt solution suitable for forming a hydrous oxide sol can be determined by simple experimentation. The minimum crystallizing temperature appears to be characteristic of the particular chemical system. The maximum crystallization temperature is limited by other practical and sometimes critical considerations. For example, the maximum crystallization temperature for urania sols in nitrate media is limited by the increase of the capacity of nitrate to oxidize uranous (+4) to the uranyl (+6) oxidation state with increasing temperature. If, for example, a non-oxidizing anion such as chloride is used, the maximum permissible crystallizing temperature would be governed, not by oxidation considerations, but by practical vapor pressure considerations, i.e., the boiling point of water or of the sol. Even this limitation can be overcome by operating a pressurized system. In some systems such as the Zr(l\/) nitrate sol, the minimum crystallizing temperature is above the boiling point of water, thus making it necessary to operate in a pressurized system in order to obtain the desired degree of crystallinity.

In addition to conductivity and temperature control, the time required to produce a given change of conductivity and the time at temperature will determine the degree to which a particular crystallization can be reproduced. For example, the amount of nitrate bound in or on a polymer species at a given conductivity is a function of the nitrate extraction time. In general, the shorter the period of nitrate extraction, the more hound nitrate will remain available for release at the onset of crystallinity. Similarly, the amount of nitrate available for release during crystallinity will determine the degree ol'eonduetivity excursion and the rate of nitrate removal during crystallization. However, the optimuni times necessary to effect each process step can be determined empirically to define a reproducible process profile.

The sols produced by following the critical operational parameters will be found to have a high degree of crystallinity. For example, uranous oxide sols produced by the method ofthis invention have consistently been produced with at least 75 percent of the contained solids crystalline. The sols are extremely stable as evidenced by the fact that their conductivity remains virtually constant over long periods, up to months, of time at room temperature. Unstable sols, i.e., those having a high amorphous-to-crystalline ratio (greater than 0.5), change perceptibly and increasingly to higher conductivity to a point where the sol eventually, over a period running to as much as several hours to several days, gels or precipitates due to the increasing generation of free nitric acid in the aqueous phase.

A most significant advantage which accrues from the method of this invention is the production ofa truly stable sol relative to sols which have been identified as stable by identifying their nitrate-to-metal mole ratio. The description of a sol by its nitrate-to-metal mole ratio alone is misleading because sol stability is governed, other factors being unchanged, by the free nitric acid rather than the nitrate-to-metal mole ratio. That is to say, as an amorphous sol crystallizes, it releases adsorbed or otherwise bound anions into the surrounding solution. The shift of nitrate and/or other anions from the bound state to the free acid state occurs with no change in over-all nitrate-to-metal ratio in the so], but it does lead to sol thickening, gelling, or to precipitation, depending on how much electrolyte is freed and how long it has been freed. On the other hand, the nitrate-to-metal ratio of a predominantly or, in the ultimate case, a fully crystalline sol is related directly to the conductivity of that so] and is an accurate index of stability since there is little anion (i.e., nitrate) released from the sol as it ages. For example, a typical, predominantly crystalline sol prepared in accordance with our invention underwent a change in conductivity of about 1,500 ,umhos/cm on aging 5.3 months at room temperature. On the other hand, a sol having a predominantly amorphous fraction underwent a change in conductivity of 6,500 ,umhos/cm in only two months.

The availability of a truly stable'sol represents a significant advantage to those users who manufacture microspheres from sols, as typified by the hydrous oxide gel microsphere process described in U. S. Pat. application Ser. No. 385,813 of common assignee now U.S. Pat. No. 3,290,122 in which inorganic microspheres are formed from a stable hydrous so] by introducing a fine stream of said hydrous sol and a surrounding stream of a dehydrating organic liquid from said sol into a droplet-forming and congealing zone. The congealed microspheres are then fired to high density. The congealed microspheres undergo considerable shrinkage in their conversion to the solid densificd microsphere. Much difficulty has been experienced where sols containing a large amorphous fraction have been used. One of the principal difficulties encountered is cracking of the spheres when they are fired to density. Manufacturers have been plagued with this problem, since they have found no way, at least prior to this invention, to standardize the quality of their starting material except in terms of relying on the nitrate-to-metal ratio of the starting sol which, as previously described, frequently does not reflect the true nature of the sol. By practicing the process of this invention it will be clear that there is now provided a predominantly crystalline sol whose conductivity accurately reflects its nitrate content and indicates the optimum nitrate level for sol stability. With such a starting sol, then, microsphere manufacturers can develop microsphere-forming techniques and firing schedules which can avoid, or at least considerably reduce, the incidence of cracking and shattering resulting from the use of sols having a deleteriously high amorphous fraction.

A typical apparatus set-up for conducting the process of this invention comprises a first vessel for containing the starting feed solution, a second vessel for regenerating the nitrate-loaded extractant consisting of an aqueous solution 1 molar in sodium carbonate and 1 molar in sodium hydroxide, and a water wash vessel for removing any entrained regenerating solution. Lines are provided for conducting fluid from the first vessel to the second and the second to the third, a return line from the third vessel for recirculating the amine extractant to the first, and a pump for circulating the amine extractant. Continuous nitrate extraction is performed by recirculating the amine reagent through the entire system with continuous regeneration of the nitrate-loaded amine. The rate of nitrate removal from the sol-forming aqueous feed solution is controlled by varying the pumping rate. The probe (CDC-104) of a Radiometer Type CDM 2d conductivity meter (Copenhagen) is maintained in the extraction vessel to monitor the conductivity of the solution as it forms a sol.

Each aqueous nitrate feed solution will generate its own characteristic conductivity-temperature profile and, before a production run, this characteristic conductivity-temperature profile must be predetermined. Such a profile is shown in FIG. 2, which represents a typical conductivity-temperature profile developed for a uranous nitrate solution as it proceeds to form a crystalline sol. Assuming the several solutions to be in their respective containers, with a protective atmosphere above each solution to prevent air oxidation of the sol, the extraction pump is turned on. In a short time, ranging from 60 to 120 minutes, the conductivity of the feed nitrate solution is taken down from point A, its initial conductivity, to point B, just above a gel line D-E, to convert the initial feed solution to a nitratedeficient condition. Any point above the gel line D-E represents a condition prior to crystallization which assures that the system is fluid and that a gel is not formed. From this point the acid-deficient solution or sol is then heated at a rate of about lC./minute to the crystallization region, 58-65C., adjusting the nitrate extraction as needed to maintain the conductivity above the gel line. Nitrate extraction is then continued or accelerated to promote crystallization. The onset of crystallization will be recognized by a sudden gas evolution and a color conversion from the characteristic dark green color ofa uranous nitrate solution to a black color, signifying the formation of the desired crystalline sol. As crystallization proceeds, the rate of nitric acid release from the polymer may exceed the extraction rate and the conductivity is seen to rise to point F. Without rapid and continuous nitrate extraction, however, the buildup of free nitric acid, and hence the conductivity, would increase to such an extent as to cause excessive oxidation of uranous species to uranyl species and inhibit crystallization. According to this invention, however, the conductivity excursion is controlled and minimized by increasing the pumping rate of the extraction liquid to a rate which effectively matches the rate of nitrate release to cause the nitrate concentration to hover about the region of crystallization. Pumping is continued at that rate until gas evolution has terminated, whereupon the nitrate extraction is conducted along the path F-G while reducing the temperature of the aqueous phase. The end point G represents a conductivity value corresponding to a nitrate-touranium ratio of 0.10 i 0.02, the optimum nitrate concentration desirable for maintaining stable U(lV) sols. Once a conductivity-temperature profile has been predetermined for a given system, it can then be used as the reference profile for producing a predominantly crystalline sol in a reproducible manner for that system.

It should be emphasized that the point F does not represent the full extent of nitrate release that normally occurs during crystallization of the so]. It represents, rather, a controlled process of nitrate removal which permits formation of a predominantly crystalline sol. Without extraction during crystallization, the conductivity would rise to a level which would prevent conversion to a predominantly crystalline stable sol.

The organic phase used in practicing the invention comprises an organic solvent and an amine selected from primary, secondary, and tertiary amines having at least 10 carbon atoms in the molecule. The tertiary amines ordinarily extract more uranium together with the nitrate than do the other amines and therefore are less desirable extractants than primary or secondary amines. The organic solvent may be any of the compounds normally used as a diluent for amines in liquidliquid extraction processes; for example, the aliphatic hydrocarbons, aromatic solvents, aromatic petroleum fractions, ketones, nitrohydrocarbons, or chlorinated solvents. The primary, secondary, and tertiary amines and diluents described as useful in U. S. Pat. No. 2,877,250, issued Mar. 10, 1959, in the name of Keith B. Brown et al., for Recovery of Uranium Values, are useful in our process. Other anion removal-methods, for example, ion-exchange, dialysis and solvent extraction with other reagents may be used as alternate techniques for effecting nitrate removal to produce a predominantly crystalline sol.

The following example illustrates specific embodiments of the invention as applied to the conversion of uranous nitrate solutions to crystalline sols. It should be noted, however, that the invention is applicable to the formation of crystalline sols from other metal nitrate solutions in which the metal is in the +4 oxidation state and further characterized by its propensity to form hywords, the specific operating parameters for any metalnitrate system within the class defined can be determined in a routine manner following the principles and instructions herein disclosed to define a characteristic conductivity-temperature profile which, in effect, characterizes a reproducible operational path for that system to produce a predominantly crystalline sol.

EXAMPLE A l,500-cc aqueous solution of L3 M U(lV), 2.6 M N0 and 0.6 M HCOOH was extracted with an organic solution consisting of a 0.25 M solution of n-lauryltrialkylmethylamine (m.w. 365) extractant a diluent comprising diethylbenzene 25% nparaffin (average m.w. The presence of formic acid has been found to reduce the tendency of the aqueous phase to emulsify in contact with the organic phase, and thus result in more clean-cut separation of the aqueous phase. The amine extraction system comprised four cylindrical settler vessels: a solvent extraction vessel containing the U(lV) solution, a regeneration vessel containing an aqueous solution 1 molar in Na CO and 1 molar in NaOH concentration, a water 3,758,670 9 iii) wash vessel, an extractant reservoir, and an extra mnt Sol density was 1.342 g/cc; sol conductivity change over 3.7 months pump. All vessels were under a protective argon temwas rg gg g ;2g? g: l yp CDM 2d All of these sols were stable over several months. conductivity meter (Copenhagen) was maintained in Moreover, the highly crystalline sols could be concenthe aqueous phase in the extraction vessel. Continuous Hated up to M Wlthout i tendency to congeal or extraction was performed by recirculating the amine In the case of molamy means gram molecular reagent through the entire system with continuous rewe'ght of metal Oxide per hter of generation. The rate of nitrate removal was controlled Electron photomlcrographs f the 9' phase of 9 by varying the pumping rate prepared by the method of our invention show the exis- The conductivity limits for gelation at given temperatence of mlcenes corislstmg of uniform Sphencal tures and the optimum temperature for crystallization glomerates of crystallites several hundred angstoms in were established for this system size, while X-ray diffraction line-broadening measure- The u(lV) nitrate Solution was extracted beginning rnents indicate a considerably smaller average crystal at 25C. During an initial extraction of nitrate the conme Thus whereas the 50nd phfise 'M {mama ductivity dropped from 72 to 27 millimhos/cm during sol prepared by the method of our invention indicated extraction, while the temperature increased from 25C. average "Ystalhte of 40 as measured by X'ray to 35C. The temperature was gradually increased at a lme broademngflthe actual d|splayed an rate of 1C. per minute, while extraction was controlled photomlcrfgmph of Sald Sohd phase Showed at a rate sufficient to permit conductivity to increase the 'f of umform agglomerates f from 250 F minimally above the gelation point. it was found that an 300 A m composed of many crystalhtes' X'ray increase of l millimholcm per 0 increase in tempep fractometry measurements showed the sol to contain ature in the range of 35-60C. prevented gelation and W0 percent crxstanme Substantially minimized u(vl) formation Dense spheroidal particals are readily produced from At about 6pc. and 45 mmimhos/cm nitrate extrac the sol products. In one case, a fully crystalline (100%) tion was increased, reducing the conductivity to 43 mil- $01, as Prepared by the methcfd of limhos and promoting crystallization. Nitrate was revennon and a $01 Prepared by concemratmgthe leased at an accelerated rate, thus causing the conduc- Sol 3 were converted to spheroldal tivity to rise rapidly. Continued nitrate extraction at an Giles by Selanon a drymg solvent and h F densl' accelerated pumping rate reduced the conductivity fled particles by Subsequent drymg and fi'rmg accorf back to the original conductivity of 45 millimhos/cm. dance Wlth the general Procedure described P Nitrate extraction was continued at to a ously mentioned Ser. No. 385,813 now U.S. Pat No. conductivity of 24 millimhos/cm after which the system 3,290,122 of common as slgnee- Selected p 9p of was allowed to cool to room temperature The Conduc the fired spheroidal particles are presented in Table II tivity decreased to 11 millimhos/cm at 25C. Nitrate 35 below' extraction as performed at 25C., after cooling overnight, to provide a conductivity of about 7 millimhos/cm, indicating a nitrate-to-uranium ratio of 0.10 i- 0.02, the optimum concentration desirable for stable ABLE II u(lV) sols made by this method. 40 Density The properties of the sol thus prepared were as fol- (QM-)1 135 $5355 lows: Final 0, 15 15, 000 size strength Sol O/U percent p.s.i. psi. (1 (g.)

U concentration (molar) 1.39 1 M 2.003 0. 002 10.78 10.81 300-350 614 u(lV) content 89 3 u 2.005 0.003 10. 53 10. 00 350400 746 No /U mole ratio 0.10 Density (8 L353 1 Measured by Hg intrusion. Shelflife (with no gelation) 5 months Change in conductivity over 5 months at room temperature 1.3 millimhos/cm Crystallinity 100 Surface area m /gram of dried gel formed from sol 136 What is claimed is: The general procedure was repeated using various L method f f astableflredominamly W starting solutions containing 0.9 to 1.3 M uranous nitallme $01 of ural'llawhlch F p irate L8 to 2 6 M N0 and 45 to 65 M HCQOHL a. heating and acid-deficient solution of uranous ni- A description of the final sols produced is summarized Q its crystallizing temperature; i T m b l b. removing free nitrate ion at a temperature in the range 5865C. at a rate which approximates the 1 ABLE I rate of nitrate release to the aqueous phase of the C00 resulting sol to promote crystallization while main- 'Im U U ay 60 taining at least percent of the total uranium in g gg xg ,312 $522 mi .1 said sol in the +4 oxidation state; and 1 1.38 B9 0.10 0.48 c. thereafter adjusting the nitrate-to-uranium mole 82 3?, ratio at a level sufficient to maintain the sol. t 1:32 85 0:15 0:41 79 2. The method according to claim 11 in which the ad- 5 34 9- 77 65 justed nitrate-to-uranium mole ratio is in the range "X-ruy crystallile sizes 3911 A. 0 08 22 "S01 density was 1.239 g/cc; sol conductivity change over 3 months was at a at an: 3.4 milIimhos/cm. 

2. The method according to claim 1 in which the adjusted nitrate-to-uranium mole ratio is in the range 0.08-0.22. 